Adding a catalyst increases the rate of reaction. If the rate increases, then either k increases, or the order of the reaction changes. Explain which specific trials you might repeat with the catalyst in order to determine which is occurring.

The consistent trial is to vary rate constant with rate of reaction, since as the the rate of reaction increases, the rate constant also increases/decreases depending on which order of reaction is taken into consideration,

Explanation:

From the Arrhenius equation

k= Ae^(-Ea/RT) , generally as catalyst is added, the activation energy(Ea) decreases and since rate constant depends essentially on temperature and Rate of reaction on both temperature and concentration

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: